An element is said to be enriched with respect to a particular isotope if it has an unnaturally large abundance of that isotope. Consider a sample of Cl2 that is enriched with 35CI 35C1 mass = 34.97 amu abundance = 85.00 % 37C1 mass = 36.97 amu abundance = 15.00 % (a) Calculate the atomic weight of the enriched Cl (b) How many Cl2 molecules are in a 0.345 g sample of the enriched chlorine?

Answer: Option (B) is the correct answer.

Explanation:

It is known that Henry's law is a relation between the concentration of a gas in a liquid (solubility) and the pressure it exerts on the surface of the liquid.

According to Henry's law, the pressure of a gas is directly proportional to the solubility of the gas in a liquid.

Henry's constant is represented by the symbol [tex]K_{H}[/tex]. And, mathematically it is represented as follows.

                      P = [tex]K_{H}C[/tex]  

where,      P = pressure and C = solubility

As the pressure for the given species is the same. Hence, the standard values of solubility of the given species is as follows.

               Gas           Solubility

                Ar          [tex]3.025 \times 10^{-5}[/tex]

               CO         [tex]2.095 \times 10^{-5}[/tex]

               Xe         [tex]10.519 \times 10^{-5}[/tex]

            [tex]CH_{3}CH_{3}[/tex]   [tex]4.556 \times 10^{-5}[/tex]

              [tex]CO_{2}[/tex]   [tex]8.21 \times 10^{-4}[/tex]

As, Henry's constant is inversely proportional to the solubility. Hence, more is the value of solubility lesser will be the value of Henry's constant.

Thus, we can conclude that out of the given options CO have the largest Henry's law constant ([tex]K_{H}[/tex]) in water.

Henry's Law constant (kH) is a measure of a gas's solubility in a liquid, with larger kH values indicating lower solubility. Therefore, Argon (Ar), a noble gas known for low solubility in water, should have the largest kH.

The Henry's Law constant (kH) is an indicator of the solubility of a gas in a liquid and is established by the nature of the gas and the solvent. According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas on the surface of the liquid. Therefore, gases with high kH values are less soluble in water because they have a lower tendency to dissolve under pressure.

Considering the given options: A) Ar B) CO C) Xe D) CH3CH3 E) CO2, the chemical compound that should have the largest Henry's Law constant (kH) in water is the one that is least soluble in water. The molecule Ar (Argon) is a noble gas, which are known for their low reactivity and low solubility in water, thus it should have the largest kH.

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The question is incomplete, complete question is:

For each trial, enter the amount of heat lost by the chemical system, qrxn.

Hints: The specific heat of water is 4.184 J/g°C.   Be careful of your algebraic sign here and remember that the change in temperature is equal to the final temperature minus the initial temperature.

qrxn = - (qwater + qcalorimeter).

The heat gained by the calorimeter water, qwater, depends on the mass of water, the specific heat of water, Cpand ΔT, while the heat gained by the calorimeter, qcalorimeter, depends on the heat capacity, C and ΔT.    

DATA :        1,      2,      3

[tex]T_i(^oC)[/tex]       24.2, 24.0 ,  23.2

[tex]T_f(^oC)[/tex]        38.2, 37.8   , 36.6

Mass (g)          70.001 , 70.008 , 70.271

Explanation:

[tex]Q=mc\Delta T[/tex]

Where:

Q = heat absorbed or heat lost

c = specific heat of substance

m = Mass of the substance  

ΔT = change in temperature of the substance

Trail 1

Heat absorbed by the water = [tex]Q_1[/tex]

Mass of water ,m,= 70.001 g

Specific heat water = c = 4.184 J/g°C

ΔT = [tex]T_f-T_i=38.2 ^oC - 24.2^oC = 14^oC[/tex]

[tex]Q_2=70.001 g\times 4.184 J/g^oC\times 14^oC=4,100.38 J[/tex]

Heat absorbed by the water is 4,100.38 J.

Trail 2

Heat absorbed by the water = [tex]Q_2[/tex]

Mass of water ,m,= 70.008 g

Specific heat water = c = 4.184 J/g°C

ΔT = [tex]T_f-T_i=37.8 ^oC - 24.0^oC = 14.2^oC[/tex]

[tex]Q_2=70.008 g\times 4.184 J/g^oC\times 14.2^oC=4,042.21 J[/tex]

Heat absorbed by the water is 4,042.21 J.

Trail 3

Heat absorbed by the water = [tex]Q_3[/tex]

Mass of water ,m,= 70.271 g

Specific heat water = c = 4.184 J/g°C

ΔT = [tex]T_f-T_i=36.6^oC - 23.2^oC = 13.4^oC[/tex]

[tex]Q_3=70.271 g\times 4.184 J/g^oC\times 13.18^oC=3939.78 J[/tex]

Heat absorbed by the water is 3,939.78 J.

Answer:

E Indium =     4.407 x 10⁻¹⁹ J

E Thallium =  3.716 x 10⁻¹⁹ J

Explanation:

From Planck´s equation for a given wavelength, the energy is given by.

E = h ( c/ λ )

h: Planck´s constant, 6.626 x 10⁻³⁴ J·s

c: light speed, 3 x 10⁸ m/s

λ: wavelength in m

We will need first to convert the given wavelengths to m:

451.1  nm x ( 1 m/10⁹  nm ) = 4.511 x 10⁻⁷  m

535.0 nm x ( 1 m/10⁹ nm ) = 5.350 x 10⁻⁷ m

E Indium =    6.626 x 10⁻³⁴  J·s x 3x 10 ⁸ m/s/ 4.511 x 10⁻⁷  m = 4.407 x 10⁻¹⁹ J

E Thallium =  6.626 x 10⁻³⁴ J·s x 3x 10 ⁸ m/s/ 5.350 x 10⁻⁷ m = 3.716 x 10⁻¹⁹ J

The question is incomplete, here is the complete question:

A chemist adds 370.0 mL of a 2.25 M iron(III) bromide solution to a reaction flask. Calculate the mass in grams of iron(III) bromide the chemist has added to the flask. Round your answer to 3 significant digits

Answer: The mass of iron (III) bromide is 246. grams

Explanation:

To calculate the mass of solute, we use the equation used to calculate the molarity of solution:

[tex]\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}[/tex]

We are given:

Molarity of solution = 2.25 M

Molar mass of iron (III) bromide = 295.6 g/mol

Volume of solution = 370.0 mL

Putting values in above equation, we get:

[tex]2.25M=\frac{\text{Mass of solute}\times 1000}{295.6\times 370.0}\\\\\text{Mass of solute}=\frac{2.25\times 295.6\times 370.0}{1000}=246.1g[/tex]

Hence, the mass of iron (III) bromide is 246. grams

Answer: 0.14g

Explanation:

Mass conc. = n x molar Mass

Mass conc. = 0.070 x 2 = 0.14g

Answer:

The mass of hydrogen gas that participates is 0.14 grams

Explanation:

Step 1: Data given

Moles of H2 = 0.070 moles

Molar mass H2 = 2.02 g/mol

Step 2: Calculate the mass of hydrogen gas

Mass of H2 = moles H2 * molar mass H2

Mass of H2 = 0.070 moles * 2.02 g/mol

Mass of H2 = 0.14 grams

The mass of hydrogen gas that participates is 0.14 grams

Explanation:

The chemical reaction equation will be as follows.

      [tex]H_{3}PO_{4} + 3NaOH \rightarrow Na_{3}PO_{4} + 3H_{2}O[/tex]

In this reaction, 1 mole of [tex]H_{3}PO_{4}[/tex] reacts with 3 mole NaOH. So, the number of moles of [tex]H_{3}PO_{4}[/tex] present  in 150 ml of 0.1 M solution is calculated as follows.

               No. of moles = [tex]\frac{150}{1000 \times 0.1}[/tex]  

                                      = 0.015 mol

As it reacts with 3 moles of NaOH. Hence, no.. of moles of NaOH are:

                           [tex]3 \times 0.015 mol[/tex]

                              = 0.045 mol

So, moles of NaOH in 400 of 0.2 M NaH is as follows.

                No. of moles = [tex]\frac{400}{1000 \times 2}[/tex]

                                       = 0.080 mol

Hence, no. of moles remained after the reaction are as follows.

                 (0.080 - 0.045) mol

               = 0.035 mol NaOH in 550 ml (400 ml + 150 ml)

As molarity is the no. of moles present in liter of solution. Hence, molarity of   NaOH is as follows.

     Molarity = [tex]\frac{\text{no. of moles}}{\text{volume in liter}}[/tex]

                    = [tex]\frac{0.035}{550}[/tex]        

                   = 0.0636 M

As, [tex][OH^{-}][/tex] = 0.0636 M. Hence, pOH will be 1.20.

As,           pH + pOH = 14

                  pH = 14 - pOH

                        = 14 - 1.20

                        = 12.80

Also, [tex][H^{+}] = 10^{-pH}[/tex]    

So,          [tex][H^{+}] = 10^{-12.80}[/tex]    

                           = [tex]1.58 \times 10^{-13}[/tex] M

Thus, we can conclude that pH of the given solution is 12.80 and its hydrogen ion concentration is [tex]1.58 \times 10^{-13}[/tex] M.

Answer:

pH = 12.80  

[H+] = 1.58 * 10^-13 M

Explanation:

Step 1: Data given

Volume of 0.2M NaOH = 400 mL

Volume of 0.1M H3PO4 = 150 mL

Step 2: The balanced equation

H3PO4 + 3NaOH → Na3PO4 + 3H2O  

For 1 mol H3PO4 we need 3 mol of NaOH to produce 1 mol Na3PO4 and 3 mol H2O

Step 3: Calculate moles H3PO4

Moles H3PO4 = molarity * volume

Moles H3PO4 = 0.1 M * 0.150 L

Moles H3PO4 = 0.015 moles

Step 4: Calculate moles NaOH

Moles NaOH = 0.2M * 0.400 L

Moles NaOH = 0.08 moles

For 1 mol H3PO4 we need 3 mol of NaOH to produce 1 mol Na3PO4 and 3 mol H2O

0.015 mol H3PO4   will react with 0.045 mol NaOH  

Step 5: Calculate moles remaining

H3PO4 will be completely consumed

There will remain 0.08 - 0.045 = 0.035 moles of NaOH

Step 6: Calculate total volume

Total volume = 400 mL + 150 mL = 550 mL = 0.550 L

Step 7: Calculate molarity of the solution

Molarity = moles / volume

Molarity = 0.035 moles / 0.550 L

Molarity = 0.0636 M NaOH

Step 8: Calculate pOH

[OH-] = 0.0636M  

pOH = -log [OH-]  

pOH = -log(0.0636)

pOH= 1.20

Step 9: Calculate pH

pH = 14.00- pOH  

pH = 14.00 - 1.20  

pH = 12.80  

[H+] = 10^-12.80

[H+] = 1.58 * 10^-13 M

Answer:

47.5 g of water can be formed

Explanation:

This is the reaction:

CH₄  +  2O₂  →  CO₂ + 2H₂O

Methane combustion.

In this process 1 mol of methane react with 2 moles of oxygen to produce 2 moles of water and 1 mol of carbon dioxide.

As ratio is 1:2, I will produce the double of moles of water, with the moles of methane I have.

1.320 mol  .2 = 2.64 moles

Now, we can convert the moles to mass (mol . molar mass)

2.64 mol . 18g/mol = 47.5 g

Answer:

mass H2O = 47.56 g

Explanation:

balanced reation:

∴ moles CH4 = 1.320 mol

⇒ moles H2O = (1.320 mol CH4)×(2 mol H2O/mol CH4)

⇒ moles H2O = 2.64 mol H2O

∴ molar mass (mm) H2O = 18.015 g/mol

⇒ mass H2O = (2.64 mol H2O)×(18.015 g/mol)

⇒ mass H2O = 47.56 g

Answer: The unknown element X is calcium.

Explanation:

We are given:

An ionic compound having chemical formula = [tex]XCl_2[/tex]

The given compound is a neutral compound and in a neutral compound, the oxidation states are exchanged.

We know that:

Oxidation state of chlorine ion = -1

So, the oxidation state of X ion will be +2

Atomic number is defined as the number of protons or electrons that are present in a neutral atom.

Atomic number = number of protons = number of electrons

Number of electrons = Number of protons - charge

We are given:

Mass number = 40

Number of electrons = 18

So, number of protons = Number of electrons + Charge

Number of protons = 18 + 2 = 20 = Atomic number

Hence, the unknown element X is calcium having atomic number '20'

The element represented by X in the compound XCl2, with a mass number of 40 and having 18 electrons in its ion, is Calcium.

The element in question is likely Calcium (Ca). Given the formula XCl2, we can infer that the element X must have a charge of +2. Since ions form when atoms gain or lose electrons to attain a stable electron configuration, and because X has 18 electrons, it must have lost 2 electrons because its neutral state would have 20 electrons (Atomic number = Protons = Electrons in a neutral atom). Now, considering the mass number (which is the sum of protons and neutrons) is 40, and knowing that it has 20 protons, it means our element has 20 neutrons. The only element that fits this profile is Calcium, which has 20 protons and is in Group 2 and commonly forms a +2 ion.

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Answer:

mol fraction HNO₃ = 0.38

mol fraction H₂O    = 0.62

Explanation:

The mole fraction of a solution is an expression of concentration given by

Xₐ = nₐ / nt

where nₐ is the number of moles of component A, and

nt is the total number of moles ( solute + solvent) present.

The number of moles we can calculate by dividing mass into molecular weight, and since we are given the concentration in percent by mass we can use this information to calculate the number of moles of the two components in the solution.

Assume 100 g of concentrated solution, so we have 68 g of HNO₃ and ( 100 - 68 ) g of H₂O.

n HNO₃ = 68 g / 63.01 g/mol = 1.08 mol HNO₃

n H₂O =     32 g/ 18.02 g/mol = 1.78 mol H₂O

nt = 1.08 mol + 1.78 mol = 2.86 mol

Now we can calculate the mol fractions:

X HNO₃ = 1.08 mol / 2.86 mol = 0.38

X H₂O =    1.78 mol / 2.86 mol = 0.62

( since the solution is binary we could also calculate the mol fraction of H₂O as 1 - X HNO₃ )

Final answer:

Water boiling is endothermic, gasoline burning is exothermic, and ice forming is exothermic.

Explanation:

a. Water boiling is an endothermic process because heat is required to convert water from the liquid to the gaseous phase. The reaction absorbs energy from the surroundings, resulting in a decrease in temperature.

b. Gasoline burning is an exothermic process because it releases heat into the surroundings. The combustion of gasoline produces energy in the form of heat and light.

c. Ice forming on a pond is an exothermic process. When liquid water freezes, it releases heat into the surroundings, resulting in a decrease in temperature.

The answer is as follows: (a) Endothermic, H > 0

(b) Endothermic, H > 0

(c) Exothermic, H < 0

Explanation and logic of the

 (a) When an ice cube melts, it absorbs heat from its surroundings to break the hydrogen bonds between water molecules, which requires energy. This process is endothermic, meaning it absorbs heat from the surroundings, and the enthalpy change (H) is positive because the system is gaining energy.

(b) Nail polish remover evaporating quickly after being spilled also involves an endothermic process. The liquid absorbs heat from the skin, causing it to change state from liquid to gas. This phase change requires energy, which is why the skin feels cooler as the nail polish remover evaporates. The enthalpy change (H) is positive because the system is gaining energy from the surroundings.

(c) Gasoline burning within the cylinder of an automobile engine is an exothermic reaction. When gasoline combusts, it releases a significant amount of energy in the form of heat and light. This energy is transferred to the surroundings, and the enthalpy change (H) is negative because the system is losing energy. This is characteristic of exothermic reactions, where the energy released is greater than the energy absorbed.

Answer:

15.95

Explanation:

This question is a modification of the calculation of  the empirical formula of a compound given its percent composition and atomic weights of the elements in the compound.

Here we are given the formula and the percent composition, so we know that there are 4 atoms of E per 2 atoms of N so lets solve using the information given.

In 100 grams of the binary compound we have

30.46 g N

69.54 g E

The number of moles is the mass divided by atomic weight:

mol N = 30.46 g / A.W N = 30.46 g / 14.00 g/mol = 2.18 mol N

mol E = 65.54 g / A.W E

Thus,

4 mol E/ 2 mol N = ( 69.54 g/ A.W E ) / 2.18

2  A.E = 65.54 g / 2.18  ⇒ A.W E = 69.54 g / ( 2 x 2.18 ) = 15.94 g

So the A.W is 15.94 g/mol which is close  the atomic weight of O.

Answer:The atomic mass of E is 51

Explanation:Please see attachment for explanation

The direction of the hydrolysis of ATP to ADP depends on the cellular conditions and the free energy change of the reaction. It is a reversible reaction, and the direction will depend on the energy requirements of the cell.

The hydrolysis of ATP to ADP is a reversible reaction. The direction in which the reaction will progress depends on the conditions. To determine this, we need to consider the free energy change (ΔG) of the reaction. In this case, the standard free energy of hydrolysis of ATP is -30.5 kJ/mol, which means that the hydrolysis reaction is exergonic and releases energy.

Since cells rely on the regeneration of ATP, the reverse reaction (regeneration of ATP from ADP + P) requires an input of free energy. The direction of the reaction will depend on the cellular conditions, such as ATP and ADP concentrations, enzyme activity, and energy requirements.

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Under standard conditions, the reaction will progress in the direction of ATP hydrolysis, meaning ATP will break down into ADP and Pi. This is due to the negative standard free energy change of -30.5 kJ/mol for ATP hydrolysis, making it exergonic. Consequently, the reverse reaction of ATP synthesis from ADP and Pi is not favored.

To determine the direction in which the reaction will progress, you need to consider the standard free energy change (
ΔG°) of the reaction. The standard free energy of hydrolysis of ATP is -30.5 kJ/mol, indicating that the hydrolysis of ATP into ADP and Pi is highly exergonic and releases energy.

Given the reaction:

If the reactants and products are present in equimolar amounts, the standard free energy change (ΔG°) for the reverse reaction (synthesizing ATP from ADP and Pi) will be +30.5 kJ/mol, making it highly endergonic.

Therefore, under standard conditions, the direction that the reaction will naturally progress is:

This means that ATP will hydrolyze into ADP and Pi rather than the reverse process of ATP synthesis.

Answer:

1. Hydrogen bond

2. Ion-ion

3. Hydrogen bond

4. London force

5. Hydrogen bond

Explanation:

Intermolecular forces are the ones that keep the molecules, or ions, together in the substance. If the substance is metal then, metallic forces are involved in it; if it's an ionic compound, then ion-ion forces are involved in it, and, if the compound is a molecule, it may have 3 different types of forces.

The force depends on the polarity of the molecule, which is given by the measure of the dipole moment. If the dipole moment is 0, the molecule is nonpolar, and if it's different from 0, it's polar. The polarity is given by the dipole moment, which is the vector sum of the dipoles of the bonds. The dipole is the difference of electronegativity between the elements of the bond.

The nonpolar molecules have a London force, which is the weakest force. The polar molecules have dipole-dipole forces, and, if the dipole is formed by hydrogen and a high electronegative element (N, O, or F), the dipole-dipole is extremely strong and it's called a hydrogen bond.

1. The water is a polar molecule because it has angular geometry, so, the dipole of the O-H bond is not canceled. Because it has the bond between H and O, the force is hydrogen bond.

2. CaCl2 is an ionic compound formed by the ions Ca+2 and Cl-, so the force is ion-ion.

3. CH3CH(CH3)OH has a polarity at the O-H bond, so as the water it has hydrogen bond.

4. CH4 has a tetrahedral geometry, and the dipole of the C-H bonds are canceled, so it's a nonpolar molecule with the London force.

5. NH3 has a pyramid trigonal geometry, and so the dipole of N-H is not canceled, so it's polar and has the bond of H with N, so, it has hydrogen bond force.

The substances H2O, CaCl2, CH3CH(CH3)OH, CH4, NH3 predominantly have hydrogen bonding, ionic bonding, hydrogen bonding, London dispersion forces, and hydrogen bonding & dipole-dipole interaction as their intermolecular forces respectively.

The predominant intermolecular forces in these substances are as follows:

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Answer:

p orbital.

Explanation:

Valence electrons are the electrons in an atom holding the very last orbital which is used in chemical bonding with other elements. Their existence could define the chemical properties of that atom.

During the first energy in ionization of an N2 molecule the molecular orbital from which the electron could be extracted is the only one with the highest energy level. Nitrogen has its outermost orbital (p) containing three valence electrons. Each orbital is only half filled, and thus it is unstable Thus, the electron mission must have been removed from p orbital.

For the first ionization energy for an N2 molecule, the molecular orbital that the electron is removed from is the p orbital.

It should be noted that valence electrons simply refer to the electrons in an atom that holds the last orbital that is required for chemical bonding with other elements.

The existence of valence electrons can define the chemical properties of that atom. For the first energy in ionization of an N2 molecule, the molecular orbital where the electron could be extracted is the p orbital since it has the highest energy level.

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The mass of MgCO₃ is 1.9g.

The balanced chemical reaction is shown below

Na₂CO₃   +   Mg(NO₃)₂     ⇒   2 NaNO₃   + MgCO₃

0.200 M   0.0450 M                                        ?

10.0           5.00 mL                                          ?

Since the volume and concentration of Mg(NO₃)₂ and Na₂CO₃  is given , we can calculate the number of moles for each of them and then determine the limiting reagent.

Convert the volume of  Mg(NO₃)₂and Na₂CO₃ to liters:

5.00 mL x ( 1 L/1000 mL ) =   5.00 x 10⁻³ L

10.00 mL x ( 1L/ 1000 mL ) = 1.000 x 10 ⁻² L

Number of  mol Mg(NO₃)₂ = ( 0.0450 mol /L  ) x 5.00 x 10⁻³ L

                                           = 2.25 x 10⁻⁴ mol Mg(NO₃)₂

Number of mol Na₂CO₃ = ( 0.200 mol / L ) x 1 x 10⁻² L  

                                        = 2.000 x 10⁻³  mol Na₂CO₃

Limiting reagent

    = 2.25 x 10⁻⁴ mol Mg(NO₃)₂ x ( 1 mol Na₂CO₃ / mol  Mg(NO₃)₂ )

      = 2.25 x 10⁻⁴ mol  Na₂CO₃ required .

Limiting reagent is Mg(NO₃)₂ since 2.25 x 10⁻⁴ mol  Na₂CO₃ is required to

react completely with  2.25 x 10⁻⁴Mg(NO₃)₂, and there's an excess.

Number of  mole  of MgCO₃ produced

= 2.25 x 10⁻⁴ mol  Mg(NO₃)₂ x ( 1 mol MgCO₃ / 1 mol Mg(NO₃)₂ )

= 2.25 x 10⁻⁴ mol  MgCO₃

Mole = mass/molar mass

Mass= Mole × molar mass

2.25 x 10⁻⁴ mol  MgCO₃ x   84.31 g/mol  = 1.90 g

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To calculate the mass of MgCO3 precipitated, determine the limiting reactant and use stoichiometry to find the moles and mass of MgCO3.

To calculate the mass of MgCO3 precipitated, we need to determine the limiting reactant in the reaction between Na2CO3 and Mg(NO3)2. First, calculate the moles of Na2CO3 and Mg(NO3)2 using their respective concentrations and volumes. Then, compare the moles of each reactant to determine which is limiting. Use the stoichiometry of the balanced equation to find the moles of MgCO3 produced. Finally, calculate the mass of MgCO3 using its molar mass.

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Answer:

Pyramid trigonal and trigonal planar, respectively.

Explanation:

The shape of a molecule is how the atoms are organized in the space, and it happens to minimize the repulsive force of the bonds and the lone pairs of electrons. Thus, in the molecules given, the two N atoms are the central atoms, because they can do the most number of bonds.

Nitrogen has 5 electrons in the valence shell, so it can do 3 bonds to be stable with 8 (octet rule), and fluorine has 7 electrons in the electron shell, so it can do 1 bond to be stable with 8.

In the molecule of N2F4, the two nitrogen do a simple bond between then, and simple bond with 2 F each, as shown below. So, each nitrogen still has 1 lone pair of electrons. To minimize it, the better shape is the pyramid trigonal.

In the molecule of N2F2, the two nitrogen do a double bond between them, and a simple bond with one F each, as shown below. They still have lone pairs, and the double bond is stiff, so it doesn't rotate. Thus, the trigonal planar shape is the better one.

N₂F₄ is expected to have a planar structure with sp3 hybridization for each nitrogen, resulting in a planar shape. N₂F₂ is likely to possess a bent or angular geometry due to lone pairs on the nitrogen atoms, also with sp3 hybridization, leading to an angular or bent shape.

The fluoro derivatives of nitrogen, N₂F₄ and N₂F₂, exhibit unique molecular geometries due to their structure and hybridization states. For N₂F₄, the molecule is expected to have a planar structure with a hybridization of sp3 for each nitrogen atom. This configuration leads to a molecular shape that can be described as planar. In contrast, N₂F₂ would likely have a bent or angular geometry due to the presence of lone pairs on the nitrogen atoms, also with an sp3 hybridization, making the overall shape angular or bent.

Final answer:

The correct order of the elements in terms of increasing electronegativity is Na, Mg, N, O, F, as metals tend to be less electronegative than nonmetals, and electronegativity generally increases across a period.

Explanation:

The question asks us to rank a series of elements in order of increasing electronegativity based on Linus Pauling's values. Electronegativity generally increases from left to right across a period in the periodic table and decreases from top to bottom within a group. Additionally, metals tend to have lower electronegativity compared to nonmetals. With this understanding, the correct ranking from least to most electronegative is: Na (alkali metal with relatively low electronegativity), Mg (alkaline earth metal with low electronegativity), N (nonmetal, higher electronegativity than metals), O (nonmetal, higher electronegativity than nitrogen), and F (halogen with the highest electronegativity).

Therefore, the correct order in terms of increasing electronegativity is option 2. Na, Mg, N, O, F.

The concentration of the pesticide DDT in the 3.7 L solution is approximately 113.51 ppm.

The mass of the solute (DDT) must be determined to calculate the concentration in parts per million (ppm).

So, the given quantities are:

Volume of solution (V) = 3.7 L

Density of solution (d) = 1.00 g/mL

Mass of DDT (m) = 4.21 × 10^-7 kg

Let's start by using the volume and density provided to determine the mass of the solution:

Mass of solution = Volume × Density

Mass of solution = 3.7 L × 1.00 g/mL = 3.7 kg

Now, we'll convert the mass of DDT to grams:

1 kg = 1000 g

Mass of DDT in grams = 4.21 × [tex]10^-^7[/tex] kg × 1000 g/kg = 4.21 × [tex]10^-^4[/tex] g

Now we can calculate the concentration in ppm:

Concentration (ppm) = (Mass of solute / Mass of solution) × 10^6

Concentration (ppm) = (4.21 × [tex]10^-^4[/tex] g / 3.7 kg) × [tex]10^-^6[/tex] ≈ 113.51 ppm

Therefore, the concentration of the pesticide DDT in the 3.7 L solution is approximately 113.51 ppm.

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The concentration of DDT in the solution is 0.1137 ppm. This calculation involved converting mass to grams, understanding the density to find out the total mass of the solution, and then using the formula for concentration in ppm.

To calculate the concentration of DDT in ppm (parts per million), you firstly need to convert the given mass of DDT into grams as ppm is typically expressed in terms of mass (g). We know that 1kg is equal to 1000g, so 4.21 x 10^-7 kg corresponding to 4.21 x 10^-4 g. We also know that the density of the solution is given to be 1g/mL, a 3.7L solution is therefore 3700 mL. So, the total mass of the solution will be 1.00 g/mL x 3700 mL = 3700 g.

Now, to get the concentration in ppm, we use the formula:

Concentration (ppm) = (mass of solute/mass of solution) x 10^6

Plugging in the values, we have:

Concentration (ppm) =

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Answer:

0.42 mg

Explanation:

It seems the question is incomplete, however I'll use values that have been found in a web search:

"A chemist adds 55.0 mL of a 1.7x10⁻⁵ M mercury(II) iodide solution to a reaction flask. Calculate the mass in milligrams of mercury(II) iodide the chemist has added to the flask. Round your answer to 2 significant digits."

Keep in mind that while the process of solving the problem remains the same, if the values in your question are different, your answer will differ as well.

First we calculate the moles of mercury (II) iodide (HgI₂):

Then we convert mmol to mg, using the molar mass (454.4 g/mol):

To figure out the mass of Mercury(II) iodide in the flask, multiple the molarity of the solution, the volume of the solution, and the molar mass of Mercury(II) iodide. Then convert the result from grams to milligrams.

It appears there's key information missing in your question. To calculate the mass of Mercury(II) iodide in the flask, we need to know the volume of the solution you've added (let's call this V and assume this is in liters) as well as the molarity (M) of the solution. Then, it's a simple unit conversion using the formula: mass = molarity x volume x molar mass of solute. The molar mass of Mercury(II) iodide (HgI2) is approximately 454.4 g/mol. Using the given molarity (M) and volume (V), the mass can be calculated, and then you'd convert this mass from grams to milligrams by multiplying by 1000.

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Answer: The value of equilibrium constant at -40°C is [tex]1.26\times 10^{-5}[/tex]

Explanation:

We are given:

Percent degree of dissociation = 0.456 %

Degree of dissociation, [tex]\alpha[/tex] = 0.00456

Concentration of [tex]N_2O_4[/tex], c = 0.15 M

The given chemical equation follows:

                       [tex]N_2O_4\rightleftharpoons 2NO_2[/tex]

Initial:                c             -

At Eqllm:         [tex]c-c\alpha[/tex]      [tex]2c\alpha[/tex]

So, equilibrium concentration of [tex]N_2O_4=c-c\alpha =[0.15-(0.15\times 0.00456)]=0.1493M[/tex]

Equilibrium concentration of [tex]NO_2=2c\alpha =[2\times 0.15\times 0.00456]=0.00137M[/tex]

The expression of [tex]K_{eq}[/tex] for above equation follows:

[tex]K_{eq}=\frac{[NO_2]^2}{[N_2O_4]}[/tex]

Putting values in above equation, we get:

[tex]K_{eq}=\frac{(0.00137)^2}{0.1493}\\\\K_{eq}=1.26\times 10^{-5}[/tex]

Hence, the value of equilibrium constant at -40°C is [tex]1.26\times 10^{-5}[/tex]

This is an incomplete question. The complete question is :

Calculate the change in internal energy (ΔE) for a system that is giving off 25.000 kJ of heat and is changing from 18.00 L to 15.00 L in volume at 1.50 atm pressure.

Answer: The change in internal energy for a system is -24544 Joules

Explanation:

According to first law of thermodynamics:

[tex]\Delta E=q+w[/tex]

[tex]\Delta E[/tex]=Change in internal energy

q = heat absorbed or released

w = work done or by the system

w = work done by the system=[tex]-P\Delta V[/tex]  {Work done on the system as the final volume is lesser than initial volume and is positive}

w =[tex]-1.50atm\times (15.00-18.00)L=4.50Latm=456Joules[/tex]  {1Latm=101.3J}

q = -25.000 kJ =[tex]-25.000\times 10^3J[/tex] {Heat released by the system is negative}

[tex]\Delta E=456J+(-25000)=-24544J[/tex]

Thus change in internal energy for a system is -24544 Joules

Answer:

The correct answer is option c. transfer of electrons from Mg to O.

Explanation:

Hello!

Let's solve this!

When Magnesium (Mg) reacts with oxygen (O), magnesium oxide is formed.

This reaction is spontaneous and occurs with oxidation number +2 of magnesium and oxidation number -2 of oxygen. It is an ionic union, so magnesium transfers its electrons to oxygen.

We conclude that the correct answer is option c. transfer of electrons from Mg to O.

The question does not contain the structures of the isomers.  The complete question is below (the structures are also in attachment)

Question:

Give one fragment in the mass spectrum and one peak in the IR spectrum that could be used to distinguish between these two isomers: (Designate which compound will show that diagnostic fragment or peak by preceding the value with the letter of the compound, i.e. "a47" or "b1730". Do not include any units.)

a) CC(CC=O)(C)C

b) C(C)C(=O)CCC

Answer:

a1730

b43

Explanation:

These two isomers a and b contain different functional groups viz., aldehyde and ketone respectively. They show different signals in their mass and IR spectra, hence, can be distinguished.

In mass spectrometer analysis, both species will undergo α-cleavage, i.e., carbonyl group will lose alkyl group next to it. Only the mass spectra of compound b will show a peak at 43 due to the loss of propyl carbocation. This peak is not observable in the mass spectra of compound a, although a peak at 44 might appear due to the McLafferty rearrangement of compound a.

IR spectra of both species contain characteristics peaks of their functional group. Ketone shows its C=O stretching peak at 1715 cm⁻¹, while aldehyde shows its C=O stretching peak at 1730 cm⁻¹ along with a should peak near 2830 to 2695 cm⁻¹ due to O=C-H stretching.

Answer:

The longest wavelength observed in the Balmer series of the H atom spectrum is 656.3 nm.

The shortest wavelength observed in the Balmer series of the H atom spectrum is 364.6 nm.

Explanation:

Using Rydberg's Equation:

[tex]\frac{1}{\lambda}=R_H\left(\frac{1}{n_i^2}-\frac{1}{n_f^2} \right )[/tex]

Where,

[tex]\lambda[/tex] = Wavelength of radiation

[tex]R_H[/tex] = Rydberg's Constant

[tex]n_f[/tex] = Higher energy level

[tex]n_i[/tex]= Lower energy level

[tex]\frac{1}{\lambda}=R_H\left(\frac{1}{n_i^2}-\frac{1}{n_f^2} \right )[/tex]

For wavelength to be longest, energy would be minimum, i.e the electron  will jump from third level to second level  :

[tex]n_f[/tex] = Higher energy level = [tex]3[/tex]  

[tex]n_i[/tex]= Lower energy level = 2 (Balmer series)

Putting the values, in above equation, we get

[tex]\frac{1}{\lambda_{Balmer}}=R_H\left(\frac{1}{2^2}-\frac{1}{3^2} \right )[/tex]

[tex]\lambda_{Balmer}=\frac{36}{5R_H}[/tex]

[tex]\lambda_{Balmer}=\frac{36}{5\times 1.097\times 10^7 m^-1}}=6.563\times 10^{-7} m=656.3 nm[/tex]

[tex]1 m =10^9 nm[/tex]

The longest wavelength observed in the Balmer series of the H atom spectrum is 656.3 nm.

For wavelength to be shortest, energy would be maximum, i.e the electron  will from infinite level to second level. :

[tex]n_f[/tex] = Higher energy level = [tex]\infty[/tex]  

[tex]n_i[/tex]= Lower energy level = 2 (Balmer series)

Putting the values, in above equation, we get

[tex]\frac{1}{\lambda_{Balmer}}=R_H\left(\frac{1}{2^2}-\frac{1}{\infty^2} \right )[/tex]

[tex]\lambda_{Balmer}=\frac{4}{R_H}[/tex]

[tex]=\frac{4}{1.097\times 10^7 m^-1}=3.646\times 10^{-7} m=364.6 nm[/tex]

The shortest wavelength observed in the Balmer series of the H atom spectrum is 364.6 nm.

Answer:1.4

Explanation:

Angle of incidence= 38°

Angle of refraction=26.3°

From Snell's law: n= sin i/sinr

sin i= 0.6157

sin r= 0.4430

n= 0.6157/0.4430=1.4

Note, n is dimensionless

Answer:

False

Explanation:

Magnesium is the element of second group and third period. The electronic configuration of magnesium is - 2, 8, 2 or [tex]1s^22s^22p^63s^2[/tex]

There are 2 valence electrons of magnesium.

Only the valence electrons are shown by dots in the Lewis structure.  

As, stated above, there are only two valence electrons of magnesium, so in the Lewis structure, two dots are made around the magnesium symbol.

Given that the electronic configuration is:- [tex]1s^22s^22p^63s^3[/tex] .

Orbital s cannot accommodate 3 electrons and also in magnesium it has [tex]3s^2[/tex] . Hence, the statement is false.

Answer:

The correct answer is option B.

Explanation:

Endothermic reactions are defined as the reactions in which energy of products is more than the energy of the reactants. In these reactions, energy is absorbed by the system.

The total enthalpy of the reaction [tex](\Delta H)[/tex] comes out to be positive.

Exothermic reactions are defined as the reactions in which energy of reactants is more than the energy of the products. In these reactions, energy is released by the system.

The total enthalpy of the reaction [tex](\Delta H)[/tex] comes out to be negative.

On mixing of both solution we had observed that temperature of the resulting solution was lowered this is because the energy was absorbed during the chemical reaction.

The true statement about the reaction is that: The chemical reaction is absorbing energy.

ENDOTHERMIC REACTION:

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The highest percent yield of N2 can be calculated by comparing the moles of N2 formed in the side reaction to the moles of N2 formed in the main reaction. In this case, the highest percent yield of N2 is 200%.

The highest percent yield of N2 that can be expected can be calculated by comparing the moles of N2 formed in the side reaction to the moles of N2 formed in the main reaction. Let's calculate:

In the side reaction, 2 moles of N2O4 produce 6 moles of NO. In this experiment, 112.4 g of N2O4 was used. So, the moles of N2O4 used is:

moles of N2O4 = mass of N2O4 / molar mass of N2O4

moles of N2O4 = 112.4 g / (92.01 g/mol) = 1.22 mol

According to the stoichiometry, 1 mole of N2 is produced for every 2 moles of N2O4 used. Therefore, the moles of N2 formed in the side reaction is:

moles of N2 = 1.22 mol / 2 = 0.61 mol

In the main reaction, 2 moles of N2H4 produce 3 moles of N2. Since the amount of N2H4 used is the same as the amount of N2O4 used (112.4 g), the moles of N2 formed in the main reaction is:

moles of N2 = 1.22 mol

Now we can calculate the highest percent yield of N2:

percent yield = (moles of N2 formed in the main reaction / moles of N2 formed in the side reaction) * 100

percent yield = (1.22 mol / 0.61 mol) * 100 = 200%

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This question requires the mass of sulfuric acid and a balance equation. The complete question is given below

Question:

According to the following reaction, how many grams of water are produced in the complete reaction of 24.1 grams of sulfuric acid?

H₂SO₄(aq) + Zn(OH)₂(s) ---------> ZnSO₄(aq) + 2H₂O(l)

Answer:

8.85 grams of water is obtained from 24.1 grams of sulfuric acid according to the given reaction

Explanation:

In this problem, the mass of water can be determined by using the balanced chemical equation.

Step 1: Write all data

Molar mass of water = 18 g

Molar mass of sulfuric acid = 98 g

Given mass of sulfuric acid = 24.1 g

Mass of water from reaction = ?

Step 2: Write statement for conversion

Given equation shows that

1 mole of H₂SO₄ gives 2 moles of water

Step 3: Convert moles into molar mass

Convert the moles into molar mass so, the statement becomes,

98 g of H₂SO₄ gives (2)(18) g of water

1 g of H₂SO₄ gives (2)(18)/98 g of water

Step 4: Use given data

24.1 g of H₂SO₄ gives (2)(18)(24.1)/98 g of water

amount of water = 8.85 g